Question

Liquid butane is used as a fuel to heat and cook with. Using the combustion of butane as your heat source, what volume (in L) of liquid butane (C4H10) must you bring with you on a three-night camping trip if you wish to heat 4.0 L of liquid water (each night) from 15.0 ºC to it’s boiling point at your camp-sight, which is at an elevation of 4000 ft? Assume the following: The state of the water formed from the combustion of butane is H2O(g) The efficiency of heat transfer from the combustion of butane to the water is 100%. The density of water at 15.0 °C is 0.9991 g/mL. The density of liquid butane is approximately 0.600 g/mL.

Answer 1

Step-by-step explanation:

mass of water to be heated = volume x density of water .

4000 x .9991 g

= 3.9964 kg

heat required per night = 3.9964 x 4.2 x ( 100 - 15 ) kJ

= 1426.71 kJ

calorific value of liquid butane = 50400 kJ / kg

so gram of liquid butane required = 1426.71 / 50400 kg

= .0283 kg

= 28.30 g

volume of liquid butane = mass / density

= 28.3 / .6

= 47.17 mL